1 mol of N2 = 28.02 g/mol

1.07 / 2.016 = 0.5308 mol H2

10.37 / 28.02 = 0.3701 mol N2

The equation states that for every mol of Nitrogen gas you need 3 moles of Hydrogen gas.

What we need to do now is find two ratio’s. First we look at the equation in order to find the coefficients. H2 has a coefficient of 3 while Nitrogen has a coefficient of 1.

So lets divide to find the ratio. 1 / 3 equals 0.333333

This is our “stoichiometric ratio”.

(Remember that the nitrogen coefficient is in the numerator, either coefficient can be in the numerator as long as you keep it in the numerator for the next step)

Now we divide the moles in the same manner to get our “Experimental ratio”. Remember we used nitrogen in the numerator above, we’ll use it in the numerator here as well.

0.3701/0.5308 = 0.697

So:

Stoichiometric ratio = 0.33333

Experimental ratio = 0.697

Compare the stoichiometric and experimental ratios:

***If the experimental ratio is the smaller one, then the reactant in the numerator of both calculations above will be called the limiting reagent.

***If the stoichiometric ratio is the smaller, then the reactant in the denominator of both calculations above will be called the limiting reagent.

As you can see the stoichiometric ratio is the smaller ratio. Therefore our limiting reagent is the Hydrogen gas.

Theoretical Yield:

Divide the coefficient of the limiting reactant 3, by the coefficient of the product 2.

3/2 = 1.5

Then multiply the number of moles of hydrogen gas by this ratio.

0.5308 mol x 1.5 = 0.7962 moles of Ammonia

For “Percent Yield” you would need to run the experiment yourself and gather the “Experimental Yield”.

Percent Yield = (Experimental Yield / Theoretical Yield) x 100

(Percent Yield is equal to Experimental Yield divided by Theoretical Yield. Multiply the decimal answer by 100 for percent.)

The only way to get Experimental yield is to run the experiment and weigh the Ammonia product. Once you have the this weight you simply divide by the molar mass of Ammonia…17.034

Its been a little while since I’ve done this actively, but this should be correct.